Chemical Kinetics Test

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Chemical Kinetics Test - 1

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Question 1
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Study of rate of chemical reaction is known as

A
Chemical change

B
Chemical equilibrium

C
Chemical thermodynamics

D
Chemical kinetics

Solution

Chemical kinetics is the branch of chemistry which deals with the study of rate of reaction, factors affecting the rate of reaction and mechanism of the chemical reaction.
Question 2
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For which of the following reaction the units of rate constant and rate of the reaction are same?

A
Third order reaction

B
Zero order reaction

C
First order reaction

D
Second order reaction

Solution

Rate = k[Reactant]⁰
Question 3
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R₁ is the rate of a simple reaction 2NO + O₂→ 2NO₂.

If the volume of the reaction vessel is doubled, the rate of the reaction becomes

A
1/8 R₁

B
8 R₁

C
R₁

D
1/2 R₁
Question 4
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The rate of reaction can be measured as

A
Rate of reaction can be measured in terms of Rate of disappearance of reactant or rate of appearance of product

B
Rate of appearance of the product

C
Rate of appearance of reactant

D
Rate of disappearance of reactant

Solution

rate of reaction = (+) rate of appearance of products = (-) rate of disappearance of reactants
Question 5
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The inversion of cane sugar is represented by C₁₂H₂₂O₁₁ + H₂O → C₆H₁₂O₆ + C₆H₁₂O₆. This reaction is a

A
second-order reaction

B
unimolecular reaction

C
pseudo-unimolecular reaction

D
None of these
Question 6
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Which among the following is an instantaneous reaction?

A
Precipitation of silver chloride.

B
Burning of a log of wood

C
Rusting of iron

D
Hydrolysis of starch

Solution

Mixing of silver nitrate and sodium chloride involves ionic reaction to form precipitates of silver chloride.

AgNO₃(aq) + NaCl(aq) → AgCl(s) + NaNO₃(aq)

Since ionic reactions are very fast, so it is an instantaneous reaction.
Question 7
1 / -0

The following question has four choices out of which ONLY ONE is correct.

Which of the following statements is not true in terms of reaction kinetics?

A
A catalyst speeds up a reaction by lowering the activation energy.

B
Rise of temperature increases the rate as the number of molecules increases.

C
Increase of concentration speeds up a reaction as it increases the collision frequency.

D
Removal of product from the reaction vessel as soon as it is formed increases the reaction rate as it increases the collision frequency of reactant molecules.
Question 8
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For the reaction 2A → 3B, the rate of reaction may be represented as

A
r = – d[A]/dt = d[B]/dt

B
r = – d[A]/dt = (1/3) d[B]/dt

C
r = – (1/2) d[A]/dt = (1/3) d[B]/dt

D
r = (1/2) d[A]/dt = – (1/3) d[B]/dt
Question 9
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A catalyst is a substance which

A
increases the equilibrium concentrations of the products

B
decreases the energy of activation

C
does not alter reaction mechanism

D
increases the frequency of collision of reacting species
Question 10
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The half-life of a second-order reaction A → B is given as

A
t_1/2 = 0.693/k

B
t_1/2 = k/[A₀]

C
t_1/2 = [A]₀/k

D
t_1/2 = 1/k[A]₀

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Re-Attempt Weekly Quiz Competition

Chemical Kinetics Test - 1

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Chemical Kinetics Test - 1

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Rank

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SHARING IS CARING

Question 1

Chemical change

Chemical equilibrium

Chemical thermodynamics

Chemical kinetics

Solution

Question 2

Third order reaction

Zero order reaction

First order reaction

Second order reaction

Solution

Question 3

1/8 R1

8 R1

R1

1/2 R1

Question 4

Rate of reaction can be measured in terms of Rate of disappearance of reactant or rate of appearance of product

Rate of appearance of the product

Rate of appearance of reactant

Rate of disappearance of reactant

Solution

Question 5

second-order reaction

unimolecular reaction

pseudo-unimolecular reaction

None of these

Question 6

Precipitation of silver chloride.

Burning of a log of wood

Rusting of iron

Hydrolysis of starch

Solution

Question 7

A catalyst speeds up a reaction by lowering the activation energy.

Rise of temperature increases the rate as the number of molecules increases.

Increase of concentration speeds up a reaction as it increases the collision frequency.

Removal of product from the reaction vessel as soon as it is formed increases the reaction rate as it increases the collision frequency of reactant molecules.

Question 8

r = – d[A]/dt = d[B]/dt

r = – d[A]/dt = (1/3) d[B]/dt

r = – (1/2) d[A]/dt = (1/3) d[B]/dt

r = (1/2) d[A]/dt = – (1/3) d[B]/dt

Question 9

increases the equilibrium concentrations of the products

decreases the energy of activation

does not alter reaction mechanism

increases the frequency of collision of reacting species

Question 10

t1/2 = 0.693/k

t1/2 = k/[A0]

t1/2 = [A]0/k

t1/2 = 1/k[A]0

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1/8 R₁

8 R₁

R₁

1/2 R₁

t_1/2 = 0.693/k

t_1/2 = k/[A₀]

t_1/2 = [A]₀/k

t_1/2 = 1/k[A]₀